A) 5.623
B) 2.903
C) 4.509
D) 3.723
Correct Answer: B
Solution :
\[[{{H}^{+}}]=\]molarity \[\times \] degree of dissociation \[=\frac{0.01\times 12.5}{100}=1.25\times {{10}^{-3}}\] We know that, \[pH=-\,\log \,[{{H}^{+}}]\] \[=-\,\log \,(1.25\times {{10}^{-3}})\] \[=-\,\log \,1.25+3\] \[=3-0.0970=2.9030\]You need to login to perform this action.
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